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Unit 4 Periodic Table
Elements are arranged in order according to increasing atomic number
Periods go across and Groups go down
Different types of elements: Alkali metals, Alkaline Earth Metals, Metalloids, Transition Metals, Non Metals, Noble Gases
Trends in Periodic Table
Electronegativity: attraction for electrons in chemical bond (higher the value, stronger the attraction.
As you move across the period, electronegativity increases. As you move down the groups, it decreases
Ionization Energy: amount of energy needed to remove loosely bound electron from gaseous atom
Increases from left to right and decreases as you go down a group.
Atomic Radius: decreases left to right and increases down a group
Shielding Effect: decrease in attraction to outer electrons to nucleus
Increases as you go down periodic table, stays the same as you move across the periodic table
Electron Affinity: same trends as electronegativity
4 different orbitals
SPDF
S- shows the shape of the orbital, can only hold a maximum of 2 electrons, 7 energy levels with S configuration
P- Nonmetals and noble gases (last row), the elements on the left and bottom of the P orbital block have less characteristics of metals
D- located in the center of the periodic table, transition metals
F- fourth energy level, can hold 14 electrons, no shape to describe them
Quantum Numbers: Describe which orbital each electron is in
Principal (n) – size of orbital (can’t be zero )
Angular (l) – Shape ( 0 , 1 , 2 , 3 )
S p d f
Magnetic (m) Quantum Number – orientation in space ( -1, 0, 1)
Spin Quantum Number – spin of axis ( - ½ , ½ )
Questions:
What is the electron configuration for Aluminum?
Which has higher electron affinity: Silicon or Oxygen?
Which type of element is each of the following (alkaline, transition…) ?
Unit 4 Periodic Table
Elements are arranged in order according to increasing atomic number
Periods go across and Groups go down
Different types of elements: Alkali metals, Alkaline Earth Metals, Metalloids, Transition Metals, Non Metals, Noble Gases
Trends in Periodic Table
Electronegativity: attraction for electrons in chemical bond (higher the value, stronger the attraction.
As you move across the period, electronegativity increases. As you move down the groups, it decreases
Ionization Energy: amount of energy needed to remove loosely bound electron from gaseous atom
Increases from left to right and decreases as you go down a group.
Atomic Radius: decreases left to right and increases down a group
Shielding Effect: decrease in attraction to outer electrons to nucleus
Increases as you go down periodic table, stays the same as you move across the periodic table
Electron Affinity: same trends as electronegativity
4 different orbitals
SPDF
S- shows the shape of the orbital, can only hold a maximum of 2 electrons, 7 energy levels with S configuration
P- Nonmetals and noble gases (last row), the elements on the left and bottom of the P orbital block have less characteristics of metals
D- located in the center of the periodic table, transition metals
F- fourth energy level, can hold 14 electrons, no shape to describe them
Quantum Numbers: Describe which orbital each electron is in
Principal (n) – size of orbital (can’t be zero )
Angular (l) – Shape ( 0 , 1 , 2 , 3 )
S p d f
Magnetic (m) Quantum Number – orientation in space ( -1, 0, 1)
Spin Quantum Number – spin of axis ( - ½ , ½ )
Questions:
- What is the electron configuration for Aluminum?
- Which has higher electron affinity: Silicon or Oxygen?
- Which type of element is each of the following (alkaline, transition…) ?
Magnesium Uranium FluorineWebsites:
http://www.chem.tamu.edu/class/majors/tutorialnotefiles/trends.htm
http://www.angelo.edu/faculty/kboudrea/general/quantum_numbers/Quantum_Numbers.htm
http://www.hhs.homewood.k12.al.us/~kreaves/Periodictable.htm